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16 Cards in this Set
- Front
- Back
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First Quantum Number |
(Principal Quantum Number) |
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The principal quantum number (n) identifies the ____ or the main energy level to which the electron belongs. |
shell |
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The value of n is a _____ . |
positive integer |
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Second Quantum Number |
(Azimuthal Quantum Number) |
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The azimuthal quantum number (l) describes the _____ of the orbital. |
shape |
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What is the shape of S, P, D, F |
Sphere Principal Diffuse Fundamental |
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value of azimuthal quantum number in S, P, D, F |
0, 1, 2, 3 |
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Third Quantum Number |
(Magnetic Orbital Quantum Number) |
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tells which particular shape of the orbital the electron occupies within an energy sublevel. |
The magnetic orbital quantum number (ml) |
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Fourth Quantum Number |
(Magnetic Spin Quantum Number) |
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(ms) describes the two ways in which an electron may be aligned in a magnetic field, parallel to or opposed to the magnetic field. The values of ms are +½ and -½. |
The magnetic spin quantum number |
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Rules in Electron Distribution |
Aufbau Principle or Building up Principle Hund’s Rule of Maximum Multiplicity Pauli’s Exclusion Principle Octet Rule |
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The sublevel in an atom is occupied by electrons in order of increasing energy level and a higher energy sublevel is not occupied until the next lower energy sublevel is fully occupied. |
Aufbau Principle or Building up Principle |
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Each orbital must be occupied by single electrons before pairing of electrons in any orbital occurs. |
Hund’s Rule of Maximum Multiplicity |
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Not more than two electrons of opposite spin can occupy an orbital. Not two electrons have the same set of quantum numbers |
Pauli’s Exclusion Principle |
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Each atom tends to acquire eight electrons in the outermost shell to become stable, except for n = 1 with 2 electrons, such as the case of Helium. |
Octet Rule |
